🤓 Based on our data, we think this question is relevant for Professor Boehr's class at PSU.
We’re being asked to calculate the lattice energy of rubidium chloride (RbCl).
Recall that lattice energy is the energy required to combine two gaseous ions into a solid ionic compound:
Mx+(g) + Ny–(g) → MyNx(s)
To calculate for lattice energy, we need to do the Born-Haber cycle for RbCl.
We start with the corresponding formation equation for RbCl:
Rb(s) + 1/2 Cl2(g) → RbCl(s), ΔH˚f
The enthalpy of formation (ΔHf) of rubidium chloride is -430.5 kJ/mol. The enthalpy of sublimation for rubidium is 86 kJ/mol, and the first ionization energy of rubidium is 402 kJ/mol. The bond dissociation energy of (g) is 243 kJ/mol, and the electron affinity of chlorine is -349 kJ/mol. Calculate the lattice energy of RbCl (s), in kJ/mol.